The activation energy for the decomposition of butene C₄H₈ in ethene C₂H₄ is 262 kJ.mol^-1.

At 300K the rate constant is 7.23 x 10^-10 s^-1.

What is the rate constant at 65.0°C?

Question

The activation energy for the decomposition of butene C₄H₈ in ethene C₂H₄ is 262 kJ.mol^-1.

At 300K the rate constant is 7.23 x 10^-10 s^-1.

What is the rate constant at 65.0°C?

| General Chemistry 2

Accepted Answer

Arrhenius equation:

k = Ae^-Ea/RT

k₂ / k₁ = Ae^-Ea/RT2 / Ae^-Ea/RT1

⇒ k₂ / k₁ = e^{-E_a/RT₂ + E_a/RT₁}

⇒ k₂ = k₁x e^{-E_a/RT₂ + E_a/RT₁}

with T₁ = 300 K and T₂ = 65.0°C = 338 K

k₂ = 9.73 x 10^-5 s^-1

Arrhenius equation - 3 | Chemical Kinetics: Mechanisms